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Question of the Day—get a calculator

Question of the Day—get a calculator. Calculate the total tuition saved if you took all 28 hours of dual credit available at FHS at the Stark State tuition rate of $135/semester credit hour. Also add in the $40 for a parking sticker And the estimated $900 for textbooks. QOD Answer.

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Question of the Day—get a calculator

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  1. Question of the Day—get a calculator • Calculate the total tuition saved if you took all 28 hours of dual credit available at FHS at the Stark State tuition rate of $135/semester credit hour. • Also add in the $40 for a parking sticker • And the estimated $900 for textbooks

  2. QOD Answer • Tuition alone = $3,780 • Including parking and books = $4,720 • How many hours would you have to work to pay off this debt if you were paid $7.50/hr? • About 630 hours • Being able to start college as almost a sophomore = priceless!

  3. 10.4 Energy Levels of Electrons Electrons move in definite energy levels; these are labeled 1 - 7

  4. Sublevels in each of the 7 main energy levels • Each level has sublevel(s) which are probability shapes or orbitals that show where the electrons may be at any one time. Also known as orbitals.

  5. S orbital can hold up to 2 electrons

  6. p sublevel can hold up to 6 electrons (2 in each orbital

  7. d sublevel can hold up to 10 electrons

  8. f sublevel can hold up to 14 electrons

  9. How do they fill? • Aufbau chart shows how electrons fill into the main energy levels and the sublevels or orbitals

  10. Energy Levels and Sublevels • 1s • 2s 2p • 3s 3p 3d • 4s 4p 4d 4f • 5s 5p 5d 5f • 6s 6p 6d 6f • 7s 7p 7d 7f

  11. Aufbau Diagram or Chart • 1s START HERE and follow • 2s 2p the arrows! • 3s 3p 3d • 4s 4p 4d 4f • 5s 5p 5d 5f • 6s 6p 6d 6f • 7s 7p 7d 7f

  12. Electron Configuration • 4 Be • 1s2 2s2 • 15 P • 1s22s22p63s23p3 • 25 Mn • 1s22s22p63s23p64s23d5

  13. Pauli Exclusion Principle • Pauli exclusion principle states that no more than 2 electrons can be in the same suborbital. Even so, this would cause them to have precisely the same quantum address. So Pauli decided there has to be a way to tell one electron from another. In other words, they must differ by at least one quantum number!

  14. Pauli Exclusion Principle • So they invented spin (+1/2 or -1/2) called spin up and spin down. Has nothing to do with the direction of the electron--we don’ t know how they move just where they may be at with 90% chance of finding it inside the energy level and orbital designated.

  15. Hund’s Rule • Hund’s rule states that electrons fill unpaired until there is no more room then they will pair (applies to p, d and f orbitals)

  16. Orbital Diagrams S orbitals get one box P orbitals get 3 boxes (2 e- per box) D orbitals get 5 boxes and f gets 7

  17. Orbital Diagrams (cont.) • Insert electrons (using arrows into each box according to Hund’s and Pauli) 2 p3

  18. Answer • 2p3 (arrows can all point up or down) • Now try 4f10

  19. Answer to 4f10 • Arrows may point up or down if they are in boxes individually; however, if there are 2 electrons in a box, one must point up and one down.

  20. Now begin working HW Handout #1

  21. Periodic Table and Periodicity You will need a calculator for QOD

  22. QOD: How much more money does a college graduate make than a high school graduate? Be sure to subtract the cost of tuition (estimate that to be about $22,000/per year for five years) and subtract out 5 years for the total time worked. Assume that the high school graduate worked from age 18 to age 68 (50 years) and earned an average income of $35,725/year, and the college graduate worked from age 23 to age 68 (45 years) and earned an average income of $57,220/year.

  23. Electrons and the Periodic Table Revisited History of the Table Periodic Law

  24. Mendeleev • Mendeleev was a Russian chemist who arranged the known elements in vertical columns in order of increasing mass and noticed a pattern in physical and chemical properties

  25. Mosley • Mosley was a British physicist who determined the atomic number (number of protons) of the atoms of elements and then arranged the elements according to their atomic number.

  26. Periods and Groups • Periods of the periodic table are the rows across • Groups or Families are columns on the periodic table. • Currently we have 18 groups. We will use the 1-18 designations not the A/B or Roman Numerals

  27. Areas of the Periodic Table • Representative elements or Main Group are those that are in Groups 1, 2, 13, 14, 15, 16, 17, 18 • Transition elements are Groups 3 - 12 , also called the Heavy Metals

  28. Inner Transition • Rare Earth elements that are located in the bottom two rows (away from the rest of the table) of the periodic table

  29. Periodic Table Main Group or Representative elements Main group GROUP NUMBERS 1 2 3 4 5 6 7 Heavy Metals or Transition elements Period Numbers Inner Transition Elements

  30. Groups with names • Group 1 = Alkali Metals • Group 2 = Alkaline Earth Metals • Group 18 = Inert or Noble Gases • Group 17 = Halogens

  31. Periodic Table and Electron Configuration • The light metals compose the s block. • The transition elements are the d block. • The nonmetals are p block. • The inner transition (rare earth) metals are the f block.

  32. Periodic Table 1 2 3 4 5 6 7 4 5 6 7 3 4 5 6 4f 5f p block Noble (inert) gases s block f block d block

  33. He 1s2 Ne 1s22s22p6 Ar = 1s22s22p63s23p6 Kr = 1s22s22p63s23p64s23d104p6 Xe = 1s22s22p63s23p64s23d104p65s24d105p6 Rn = 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6 Except He, do you see a trend in all of the noble gas configurations? What do they all end in? Complete the electron configurations for the Noble Gases (Hint: Group 18)

  34. Shorthand Notation • We use the noble gases in shorthand notation • Find the closest noble gas that has an atomic number LESS than that of the element

  35. Example • Ex. K • What is K’s atomic number? • 19 • Closest noble gas? • Ar • What is Ar’s atomic number? • 18 = 1s22s22p63s23p6 • = [Ar] 4s1 = Means the first 18 electrons are arranged like argon and the last electron is called the VALENCE ELECTRON (outermost shell)

  36. Example for you to try • You try Ba • Ba = [Xe] 6s2 • Try Pb • Pb = [Xe] 6s24f145d106p2

  37. Valence Electrons • The electrons after the noble (inert) gas configuration • Electrons in the highest occupied energy levels • Give the characteristics or chemical properties of the element

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